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Questions and Answers
How does a decomposition reaction differ fundamentally from a combination reaction?
How does a decomposition reaction differ fundamentally from a combination reaction?
A decomposition reaction involves breaking down a compound into simpler substances, while a combination reaction involves forming a compound from simpler substances.
What type of energy is commonly required to initiate a decomposition reaction, and why is it necessary?
What type of energy is commonly required to initiate a decomposition reaction, and why is it necessary?
Decomposition reactions commonly require an input of energy such as heat, light, or electricity. This energy is needed to break the chemical bonds holding the compound together.
If a binary compound decomposes, what are the expected products? Provide a general example.
If a binary compound decomposes, what are the expected products? Provide a general example.
The expected products are the two elements that make up the binary compound. For example, the decomposition of water (H₂O) yields hydrogen (H₂) and oxygen (O₂).
Predict the products of the decomposition of aluminum oxide ($Al_2O_3$).
Predict the products of the decomposition of aluminum oxide ($Al_2O_3$).
What products are typically formed when a metal carbonate undergoes decomposition?
What products are typically formed when a metal carbonate undergoes decomposition?
Write a balanced chemical equation for the decomposition of copper(II) carbonate ($CuCO_3$).
Write a balanced chemical equation for the decomposition of copper(II) carbonate ($CuCO_3$).
What are the products when metal hydroxides are heated?
What are the products when metal hydroxides are heated?
Describe the decomposition of carbonic acid ($H_2CO_3$) and name the products.
Describe the decomposition of carbonic acid ($H_2CO_3$) and name the products.
Besides heat, what other forms of energy can be used to initiate decomposition reactions?
Besides heat, what other forms of energy can be used to initiate decomposition reactions?
Is the reaction $2H_2O(l) → 2H_2(g) + O_2(g)$ a decomposition reaction? Explain why or why not.
Is the reaction $2H_2O(l) → 2H_2(g) + O_2(g)$ a decomposition reaction? Explain why or why not.
What is required for a reaction to be classified as a combustion reaction?
What is required for a reaction to be classified as a combustion reaction?
Name the two products that are always produced during the complete combustion of a hydrocarbon.
Name the two products that are always produced during the complete combustion of a hydrocarbon.
Explain why burning wood is considered a combustion reaction.
Explain why burning wood is considered a combustion reaction.
What kind of reaction is this: $CH_4 + 2O_2 → CO_2 + 2H_2O$?
What kind of reaction is this: $CH_4 + 2O_2 → CO_2 + 2H_2O$?
If a substance burns in oxygen to produce carbon monoxide ($CO$) instead of carbon dioxide, is it still considered a combustion reaction? Explain briefly.
If a substance burns in oxygen to produce carbon monoxide ($CO$) instead of carbon dioxide, is it still considered a combustion reaction? Explain briefly.
How can you differentiate between the decomposition of a metal hydroxide and the combustion of a hydrocarbon based on their products?
How can you differentiate between the decomposition of a metal hydroxide and the combustion of a hydrocarbon based on their products?
Is the reverse of a combustion reaction (i.e., combining $CO_2$ and $H_2O$ to form a hydrocarbon and $O_2$) a feasible process under normal conditions? Why or why not?
Is the reverse of a combustion reaction (i.e., combining $CO_2$ and $H_2O$ to form a hydrocarbon and $O_2$) a feasible process under normal conditions? Why or why not?
If you heat calcium carbonate ($CaCO_3$) strongly, what two products will be formed?
If you heat calcium carbonate ($CaCO_3$) strongly, what two products will be formed?
What is the key difference in the products formed when decomposing a metal oxide versus a metal carbonate?
What is the key difference in the products formed when decomposing a metal oxide versus a metal carbonate?
Consider the reaction: $2KClO_3(s) → 2KCl(s) + 3O_2(g)$. Is this a decomposition reaction? Explain your answer briefly.
Consider the reaction: $2KClO_3(s) → 2KCl(s) + 3O_2(g)$. Is this a decomposition reaction? Explain your answer briefly.
Flashcards
Decomposition Reaction
Decomposition Reaction
A reaction where a compound breaks down into two or more simpler substances.
General Form of Decomposition
General Form of Decomposition
AB → A + B, where a compound (AB) breaks down into simpler substances (A and B).
Decomposition of Binary Compounds
Decomposition of Binary Compounds
Breaking down a compound of two elements into those individual elements.
Products of Metal Oxide Decomposition
Products of Metal Oxide Decomposition
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Products of Non-Metal Oxide Decomposition
Products of Non-Metal Oxide Decomposition
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Products of Metal Carbonate Decomposition
Products of Metal Carbonate Decomposition
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Products of Metal Hydroxide Decomposition
Products of Metal Hydroxide Decomposition
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Products of Unstable Acid Decomposition
Products of Unstable Acid Decomposition
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Combustion Reaction
Combustion Reaction
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Products of Combustion
Products of Combustion
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Study Notes
- Decomposition reactions involve a compound breaking down into two or more simpler substances.
- The general form of a decomposition reaction is AB → A + B.
- Decomposition reactions are the direct opposite of combination reactions.
- Most decomposition reactions require an input of energy such as heat, light, or electricity.
Decomposition of Binary Compounds
- Binary compounds, which consist of two elements, can decompose into their elements.
- Mercury oxide (HgO) decomposes when heated into mercury (Hg) and oxygen gas (O₂).
- When decomposing a metal oxide, the products are a metal element and oxygen gas (O₂).
- When decomposing a non-metal oxide, the products are a non-metal and oxygen gas (O₂).
Decomposition into Other Compounds
- A reaction is still a decomposition reaction even if some products are compounds.
- Metal carbonates decompose into metal oxides and carbon dioxide gas (CO₂).
- Calcium carbonate (CaCO₃) decomposes into calcium oxide (CaO) and carbon dioxide (CO₂).
- Metal hydroxides decompose on heating to yield metal oxides and water (H₂O).
- Sodium hydroxide (NaOH) decomposes to produce sodium oxide (Na₂O) and water (H₂O).
- Unstable acids decompose to produce non-metal oxides and water.
- Carbonic acid (H₂CO₃) decomposes into carbon dioxide (CO₂) and water (H₂O) at room temperature.
Combustion Reactions
- Combustion reactions occur when a substance reacts with oxygen gas (O₂), releasing energy as light and heat.
- Combustion reactions must involve oxygen gas as a reactant.
- Combustion is also known as burning (e.g., burning matches, candles, campfires, and gas burners).
- The products of a combustion reaction are always carbon dioxide (CO₂) and water vapor (H₂O).
- Burning naphthalene (C₁₀H₈) produces carbon dioxide (CO₂) and water vapor (H₂O).
- The combustion of ethane (C₂H₆) produces carbon dioxide (CO₂) and water vapor (H₂O).
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